Calculate Δ G° for the following cell reaction Zn(s) +Ag2O(s) +H2O(l) - Zn2+n(aq) +2Ag(s) +2-OH(aq) E°Ag+/Ag=+0.80V and E°Zn2+/Zn=-0.76 V

Question

Calculate Δ G° for the following cell reaction Zn(s) +Ag2O(s) +H2O(l) -> Zn2+n(aq) +2Ag(s) +2-OH(aq) E°Ag+/Ag=+0.80V and E°Zn2+/Zn=-0.76 V  (A)  - 305 kJ/mol  (B)  -301 kJ/mol  (C)  305 kJ/mol  (D)  301 kJ/mol

Tardigrade Admin · Accepted Answer

Given that, E° Ag + / Ag =+0.80 V E° Zn 2+ / Zn =-0.76 V E Cell ° =E R °-E° L =0.80-(-0.76)=1.56 V From the equation Δ G°=-n F E° (where, F=96500, n=2 ) =-2 × 96500 × 1.56 =-301080 J / mol =-301.080 kJ / mol =-301 kJ / mol

Q. Calculate $Δ G^{\circ}$ for the following cell reaction
$Zn X_{(s)} + Ag X_{2} O X_{(s)} + H X_{2} O X_{(l)}$
$Zn X_{n (aq)}^{2 +} + 2 Ag X_{(s)} + 2 X^{-} OH X_{(aq)}$
$E_{A g^{+} / A g}^{\circ} = + 0.80 V$ and $E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V$

$- 305 k J / m o l$

$- 301 k J / m o l$

$305 k J / m o l$

$301 k J / m o l$

Q. Calculate ΔG∘ for the following cell reaction ZnX(s)​​+AgX2​OX(s)​​+HX2​OX(l)​​​ ZnXn(aq)​2+​+2AgX(s)​​+2X−OHX(aq)​​ EAg+/Ag∘​=+0.80V and EZn2+/Zn∘​=−0.76V

−305kJ/mol

−301kJ/mol

305kJ/mol

301kJ/mol

Given that, E∘Ag+/Ag=+0.80V E∘Zn2+/Zn=−0.76V ECell∘​=ER∘​−E∘L=0.80−(−0.76)=1.56V From the equation ΔG∘=−nFE∘ (where, F=96500,n=2 ) =−2×96500×1.56 =−301080J/mol=−301.080kJ/mol =−301kJ/mol

Q. Calculate $Δ G^{\circ}$ for the following cell reaction
$Zn X_{(s)} + Ag X_{2} O X_{(s)} + H X_{2} O X_{(l)}$
$Zn X_{n (aq)}^{2 +} + 2 Ag X_{(s)} + 2 X^{-} OH X_{(aq)}$
$E_{A g^{+} / A g}^{\circ} = + 0.80 V$ and $E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V$

$- 305 k J / m o l$

$- 301 k J / m o l$

$305 k J / m o l$

$301 k J / m o l$